Strontium oxide
From Wikipedia, the free encyclopedia
| Strontium oxide[1] | |
|---|---|
 |
|
 |
|
| IUPAC name |
|
| Other names | Strontia |
| Identifiers | |
| CAS number | [] |
| Properties | |
| Molecular formula | SrO |
| Molar mass | 103.62 g/mol |
| Appearance | colorless cubic crystals |
| Density | 4.70 g/cm3 |
| Melting point |
2531°C |
| Boiling point |
> 3000 °C (decomp) |
| Solubility in water | reacts, forms Sr(OH)2 |
| Solubility | miscible with caustic potash slightly soluble in alcohol insoluble in acetone and ether |
| Refractive index (nD) | 1.810 [2] |
| Structure | |
| Crystal structure | Halite (cubic), cF8 |
| Space group | Fm3m, No. 225 |
| Coordination geometry |
Octahedral (Sr2+); octahedral (O2–) |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
-592.0 kJ·mol-1 |
| Standard molar entropy S |
57.2 J·mol-1·K-1 |
| Specific heat capacity, C | 44.3 J·mol-1·K-1 |
| Hazards | |
| EU Index | Not listed |
| Flash point | Non-flammable |
| Related compounds | |
| Other anions | Strontium sulfide |
| Other cations | Beryllium oxide Magnesium oxide Calcium oxide Barium oxide |
| Related compounds | Strontium hydroxide |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox references |
|
Strontium oxide or strontia, SrO, is formed when strontium reacts with oxygen. Burning strontium in air results in a mixture of strontium oxide and strontium nitride. It also forms from the decomposition of strontium carbonate SrCO3. It is a strongly basic oxide.
Contents |
[edit] Uses
About 8% by weight of television picture tube glass is strontium oxide, which has been the major use of strontium since 1970. Color televisions and other devices containing color cathode ray tubes sold in the United States are required by law to use strontium in the faceplate to block X-ray emission. (Lead oxide can be used in the neck and funnel, but causes discoloration when used in the faceplate.)
[edit] Reactions
Elemental strontium is formed when strontium oxide is heated with aluminium in a vacuum.[1]
[edit] References
- ^ a b Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 4-87, ISBN 0849305942
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
[edit] External links
|
|||||
 |
This inorganic compound-related article is a stub. You can help Wikipedia by expanding it. |
